A saturated solution of iodine in water contain 0.330g I_(2) per litre. More than this I_(2) can be dissolved in KI solution because of the following equilibrium. I_(2(g))+I^(-)hArrI_(3)^(-) A 0.100 M KI solution actually dissolves 12.5 g "iodine per litre", most of which is converted to I_(3)^(-). Assuming that the concentration of I_(2) in all saturated solution is the same, calculate the equilibrium constant for the above reaction. What is the effect of adding water to a clear saturated solution of I_(2) in the KI solution?

A saturated solution of iodine in water contain 0.330g I_(2) per litre

1.	A saturated solution of iodine in water contain 0.330g I_(2) per litre. More than this I_(2) can be dissolved in KI solution because of the following equilibrium. I_(2(g))+I^(-)hArrI_(3)^(-) A 0.100 M KI solution actually dissolves 12.5 g "iodine per litre", most of which is converted to I_(3)^(-). Assuming that the concentration of I_(2) in all saturated solution is the same, calculate the equilibrium constant for the above reaction. What is the effect of adding water to a clear saturated solution of I_(2) in the KI solution?
Answer» SOLUTION :`707 LITRE MOL^(-1)` ,